Ccl 1110 1st Edition Exam #2 Study GuideEquations to KnowChapter 5 Equations•w = F x d •work = force x distance•DeltaE = E final - E initial•H = E +PV•Enthalpy = internal energy + (pressure x volume)Chapter 10 Equations•P1V1/T1 = P2V2/T2•Combined gas law, shows how P, V, & T are related for a constant n•r1/r2 = square root (M2/M1)•Rates of effusion = square root of molar massesChapter 15 Equations•Kc = [D]d[E]e/ [A]a[B]b•Equilibrium constant expression for a general reaction. Concentrations only; products/reactants•Kp = (Pressure D)d(Pressure E)e/ (Pressure A)a(Pressure B)b•Equilibrium constant expression in terms of partial pressures•Qc = [D]d[E]e/ [A]a[B]b•Reaction quotient; concentrations are for any time during a reaction. If the concentrations are equilibrium concentrations, then Qc = KcConcepts to KnowChapter 5•Energy (kinetic vs potential)•System vs surroundings•Internal energy & heat (relating change in internal energy to heat & work, including sign conversions)•State functions (i.e. enthalpy, internal energy, etc)•PV work (gas expansion & compression)•Exothermic & Endothermic reactions (sign changes)•Enthalpies of reaction and calculating amount of heat using thermochemical equations•Heat capacity•C = q/ delta T•Specific heat capacity•q = Cs x m x delta T•Calorimetry & bomb calorimetry•Hess’ Law•Enthalpies of formation & reaction•Nutritional Calorie, fuel valueChapter 10•Pressure unit conversions & manometer•Gas law•PV = nRT•Calculating density & molar mass•Partial pressure & mole fraction•P(total) = P(gas) +P(H2O)•Kinetic molecular theory, molecular speed & effusion•Real gasesChapter 15•Concept of equilibrium •Equilibrium constant - K•Kp & Kc relationship•Heterogeneous equilibrium•Le Chatelier’s